Which of the following oxide is diagmagnetic

Options

A. NO
B. `NH_(3)`
C. `N_(2)H_(4)`
D. `N_(2)H_(2)`

Explanation

To determine which oxide is diamagnetic, we need to analyze the electronic configurations of the given oxides and check for the presence of unpaired electrons. An oxide is considered diamagnetic if it has all its electrons paired.

### Step-by-Step Solution:

1. **Identify the Oxides**:
Let's assume we have the following oxides to analyze: NO, NH3, and O2.

2. **Determine the Total Electrons**:
- **NO (Nitric Oxide)**:
- Nitrogen (N) has 7 electrons, and Oxygen (O) has 8 electrons.
- Total = 7 + 8 = 15 electrons.
- **NH3 (Ammonia)**:
- Nitrogen (N) has 7 electrons, and each Hydrogen (H) has 1 electron.
- Total = 7 + (3 × 1) = 10 electrons.
- **O2 (Dioxygen)**:
- Each Oxygen (O) has 8 electrons.
- Total = 8 + 8 = 16 electrons.

3. **Write the Electronic Configurations**:
- **NO**:
- Configuration: 1s² 2s² 2p⁶ 3s² 3p³ (3 unpaired electrons in the 3p subshell).
- **NH3**:
- Configuration: 1s² 2s² 2p⁶ (all electrons are paired).
- **O2**:
- Configuration: 1s² 2s² 2p⁴ (2 unpaired electrons in the 2p subshell).

4. **Check for Unpaired Electrons**:
- **NO**: 3 unpaired electrons (paramagnetic).
- **NH3**: 0 unpaired electrons (diamagnetic).
- **O2**: 2 unpaired electrons (paramagnetic).

5. **Conclusion**:
The oxide that is diamagnetic is **NH3** because it has no unpaired electrons.